?Calculate the mass of each sample. a. 15.7 mol \(\mathrm{HNO}_{3}\) b. \(1.04 \times

What is the difference between an empirical formula and a molecular formula?

How do you determine how many dots to put around the Lewis symbol of an element?

Describe the octet rule in the Lewis model.

According to the Lewis model, what is a chemical bond?

How can you use Lewis structures to determine the formula of ionic compounds? Give an example.

What is lattice energy?

Why is the formation of solid sodium chloride from solid sodium and gaseous chlorine exothermic, even though it takes more energy to form the \(Na^{+}\) ion than the amount of energy released upon formation of \(Cl^{-}\)? Text Transcription: Na^+ Cl^-

Explain how to write a formula for an ionic compound given the names of the metal and nonmetal (or polyatomic ion) in the compound.

Explain how to name binary ionic compounds. How do you name an ionic compound if it contains a polyatomic ion?

Why do the names of some ionic compounds include the charge of the metal ion while others do not?

Within a covalent Lewis structure, what is the difference between lone pair and bonding pair electrons?

In what ways are double and triple covalent bonds different from single covalent bonds?

How does the Lewis model for covalent bonding account for why certain combinations of atoms are stable while others are not?

How does the Lewis model for covalent bonding account for the relatively low melting and boiling points of molecular compounds (compared to ionic compounds)?

Explain how to name molecular inorganic compounds.

How many atoms are specified by each of these prefixes: mono, di, tri, tetra, penta, hexa?

What is the formula mass for a compound? Why is it useful?

Explain how the information in a chemical formula can be used to determine how much of a particular element is present in a given amount of a compound. Provide some examples of how this might be useful.

What is mass percent composition? Why is it useful?

Which kinds of conversion factors are inherent in chemical formulas? Provide an example.

Which kind of chemical formula can be obtained from experimental data showing the relative masses of the elements in a compound?

How can a molecular formula be obtained from an empirical formula? What additional information is required?

What is combustion analysis? What is it used for?

Which elements are normally present in organic compounds?

Classify each compound as ionic or molecular. a. \(\mathrm{CO}_{2}\) b. \(\mathrm{NiCl}_{2}\) c. NaI d. \(\mathrm{PCl}_{3}\) Text Transcription: CO_2 NiCl_2 PCl_3

Classify each compound as ionic or molecular. a. \(\mathrm{CF}_{2} \mathrm{Cl}_{2}\) b. \(\mathrm{CCl}_{4}\) c. \(\mathrm{PtO}_{2}\) d. \(\mathrm{SO}_{3}\) Text Transcription: CF_2Cl_2 CCl_4 PtO_2 SO_3

Determine the empirical formula for the compound represented by each molecular formula. a. \(\mathrm{N}_{2} \mathrm{O}_{4}\) b. \(\mathrm{C}_{5} \mathrm{H}_{12}\) c. \(\mathrm{C}_{4} \mathrm{H}_{10}\) Text Transcription: N_2O_4 C_5H_12 C_4H_10

Determine the empirical formula for the compound represented by each molecular formula. a. \(\mathrm{C}_{2} \mathrm{H}_{4}\) b. \(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}\) c. \(\mathrm{NH}_{3}\) Text Transcription: C_2H_4 C_6H_12O_6 NH_3

Determine the number of each type of atom in each formula. a. \(\mathrm{Mg}_{3}\left(\mathrm{PO}_{4}\right)_{2}\) b. \(\mathrm{BaCl}_{2}\) c. \(\mathrm{Fe}\left(\mathrm{NO}_{2}\right)_{2}\) d. \(\mathrm{Ca}(\mathrm{OH})_{2}\) Text Transcription: Mg_3(PO_4)_2 BaCl_2 Fe(NO_2)_2 Ca(OH)_2

Determine the number of each type of atom in each formula. a. \(\mathrm{Ca}\left(\mathrm{NO}_{2}\right)_{2}\) b. \(\mathrm{CuSO}_{4}\) c. \(\mathrm{Al}\left(\mathrm{NO}_{3}\right)_{3}\) d. \(\mathrm{Mg}\left(\mathrm{HCO}_{3}\right)_{2}\) Text Transcription: Ca(NO_2)_2 CuSO_4 Al(NO_3)_3 Mg(HCO_3)_2

How do the properties of compounds compare to the properties of the elements from which they are composed?

What is a chemical bond? Why do chemical bonds form?

Explain the difference between an ionic bond and a covalent bond.

List and describe the different ways to represent compounds. Why are there so many?

Write a chemical formula for each molecular model. (See Appendix II A for color codes.)

Write a chemical formula for each molecular model. (See Appendix II A for color codes.)

Write an electron configuration for N. Then write a Lewis symbol for N and show which electrons from the electron configuration are included in the Lewis symbol.

Write an electron configuration for Ne. Then write a Lewis symbol for Ne and show which electrons from the electron configuration are included in the Lewis symbol.

Write a Lewis symbol for each atom or ion. a. Al b. \(\mathrm{Na}^{+}\) c. Cl d. \(\mathrm{Cl}^{-}\) Text Transcription: Na^+ Cl^-

Write a Lewis symbol for each atom or ion. a. \(\mathrm{S}^{2-}\) b. Mg c. \(\mathrm{Mg}^{2+}\) d. P Text Transcription: S^2- Mg^2+

Write the Lewis symbols that represent the ions in each ionic compound. a. NaF b. CaO c. \(\mathrm{SrBr}_{2}\) d. \(\mathrm{K}_{2} \mathrm{O}\) Text Transcription: SrBr_2 K_2O

Write the Lewis symbols that represent the ions in each ionic compound. a. SrO b. \(\mathrm{Li}_{2} \mathrm{S}\) c. \(\mathrm{CaI}_{2}\) d. RbF Text Transcription: Li_2 S CaI_2

Use Lewis symbols to determine the formula for the compound that forms between each pair of elements. a. Sr and Se b. Ba and Cl c. Na and S d. Al and O

Use Lewis symbols to determine the formula for the compound that forms between each pair of elements. a. Ca and N b. Mg and I c. Ca and S d. Cs and F

The lattice energy of CsF is -744 kJ/mol, whereas that of BaO is -3029 kJ/mol. Explain this large difference in lattice energy

Rubidium iodide has a lattice energy of -617 kJ/mol, while potassium bromide has a lattice energy of -671 kJ/mol. Why is the lattice energy of potassium bromide more exothermic than the lattice energy of rubidium iodide?

Write a formula for the ionic compound that forms between each pair of elements. a. calcium and oxygen b. zinc and sulfur c. rubidium and bromine d. aluminum and oxygen

Write a formula for the ionic compound that forms between each pair of elements. a. silver and chlorine b. sodium and sulfur c. aluminum and sulfur d. potassium and chlorine

Write a formula for the compound that forms between calcium and each polyatomic ion. a. hydroxide b. chromate c. phosphate d. cyanide

Write a formula for the compound that forms between potassium and each polyatomic ion. a. carbonate b. phosphate c. hydrogen phosphate d. acetate

Name each ionic compound. a. \(\mathrm{Mg}_{3} \mathrm{N}_{2}\) b. KF c. \(\mathrm{Na}_{2} \mathrm{O}\) d. \(\mathrm{Li}_{2} \mathrm{S}\) e. CsF f. KI Text Transcription: Na_2O Mg_3N_2 Li_2S

Name each ionic compound. a. \(\mathrm{SnCl}_{4}\) b. \(\mathrm{PbI}_{2}\) c. \(\mathrm{Fe}_{2} \mathrm{O}_{3}\) d. \(\mathrm{CuI}_{2}\) e. \(\mathrm{HgBr}_{2}\) f. \(\mathrm{CrCl}_{2}\) Text Transcription: SnCl_4 PbI_2 Fe_2O_3 CuI_2 HgBr_2 CrCl_2

Name each ionic compound. a. SnO b. \(\mathrm{Cr}_{2} \mathrm{S}_{3}\) c. RbI d. \(\mathrm{BaBr}_{2}\) Text Transcription: Cr_2S_3 BaBr_2

Name each ionic compound. a. BaS b. \(\mathrm{FeCl}_{3}\) c. \(\mathrm{PbI}_{4}\) d. \(\mathrm{SrBr}_{2}\) Text Transcription: FeCl_3 PbI_4 SrBr_2

Name each ionic compound containing a polyatomic ion. a. \(\mathrm{CuNO}_{2}\) b. \(\mathrm{Mg}\left(\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\right)_{2}\) c. \(\mathrm{Ba}\left(\mathrm{NO}_{3}\right)_{2}\) d. \(\mathrm{Pb}\left(\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\right)_{2}\) Text Transcription: CuNO_2 Mg(C_2H_3O_2)_2 Ba(NO_3)_2 Pb(C_2H_3O_2)_2

Name each ionic compound containing a polyatomic ion. a. \(\mathrm{Ba}(\mathrm{OH})_{2}\) b. \(\mathrm{NH}_{4} \mathrm{I}\) c. \(\mathrm{NaBrO}_{4}\) d. \(\mathrm{Fe}(\mathrm{OH})_{3}\) Text Transcription: Ba(OH)_2 NH_4I NaBrO_4 Fe(OH)_3

Write the formula for each ionic compound. a. sodium hydrogen sulfite b. lithium permanganate c. silver nitrate d. potassium sulfate e. rubidium hydrogen sulfate f. potassium hydrogen carbonate

Write the formula for each ionic compound. a. copper(II) chloride b. copper(I) iodate c. lead(II) chromate d. calcium fluoride e. potassium hydroxide f. iron(II) phosphate

Write the name from the formula or the formula from the name for each hydrated ionic compound. a. \(\mathrm{CoSO}_{4} \cdot 7 \mathrm{H}_{2} \mathrm{O}\) b. iridium(III) bromide tetrahydrate c. \(\mathrm{Mg}\left(\mathrm{BrO}_{3}\right)_{2} \cdot 6 \mathrm{H}_{2} \mathrm{O}\) d. potassium carbonate dihydrate Text Transcription: CoSO_4 dot 7H_2O Mg(BrO_3)_2 dot 6H_2O

Write the name from the formula or the formula from the name for each hydrated ionic compound. a. cobalt(II) phosphate octahydrate b. \(\mathrm{BeCl}_{2} \cdot 2 \mathrm{H}_{2} \mathrm{O}\) c. chromium(III) phosphate trihydrate d. \(\mathrm{LiNO}_{2} \cdot \mathrm{H}_{2} \mathrm{O}\) Text Transcription: BeCl_2 dot 2H_2O LiNO_2 dot H_2O

Use covalent Lewis structures to explain why each element (or family of elements) occurs as diatomic molecules. a. hydrogen b. the halogens c. oxygen d. nitrogen

Use covalent Lewis structures to explain why the compound that forms between nitrogen and hydrogen has the formula \(\mathrm{NH}_{3}\). Show why \(\mathrm{NH}_{2}\) and \(\mathrm{NH}_{4}\) are not stable. Text Transcription: NH_3 NH_2 NH_4

Name each molecular compound. a. CO b. \(\mathrm{NI}_{3}\) c. \(\mathrm{SiCl}_{4}\) d. \(\mathrm{N}_{4} \mathrm{Se}_{4}\) Text Transcription: NI_3 SiCl_4 N_4Se_4

Name each molecular compound. a. \(\mathrm{SO}_{3}\) b. \(\mathrm{SO}_{2}\) c. \(\mathrm{BrF}_{5}\) d. NO Text Transcription: SO_3 SO_2 BrF_5

Write a formula for each molecular compound. a. phosphorus trichloride b. chlorine monoxide c. disulfur tetrafluoride d. phosphorus pentafluoride

Write a formula for each molecular compound. a. boron tribromide b. dichlorine monoxide c. xenon tetrafluoride d. carbon tetrabromide

Name each compound. (Refer to the nomenclature flowchart found in the Key Concepts section of the Chapter in Review.) a. \(\mathrm{SrCl}_{2}\) b. \(\mathrm{SnO}_{2}\) c. \(\mathrm{P}_{2} \mathrm{S}_{5}\) Text Transcription: SrCl_2 SnO_2 P_2S_5

Name each compound. (Refer to the nomenclature flowchart found in the Key Concepts section of the Chapter in Review.) a. \(\mathrm{B}_{2} \mathrm{Cl}_{2}\) b. \(\mathrm{BaCl}_{2}\) c. \(\mathrm{CrCl}_{3}\) Text Transcription: B_2Cl_2 BaCl_2 CrCl_3

Name each compound. (Refer to the nomenclature flowchart found in the Key Concepts section of the Chapter in Review.) a. \(\mathrm{KClO}_{3}\) b. \(\mathrm{I}_{2} \mathrm{O}_{5}\) c. \(\mathrm{PbSO}_{4}\) Text Transcription: KClO_3 I_2O_5 PbSO_4

Name each compound. (Refer to the nomenclature flowchart found in the Key Concepts section of the Chapter in Review.) a. \(\mathrm{XeO}_{3}\) b. KClO c. \(\mathrm{CoSO}_{4}\) Text Transcription: XeO_3 KClO CoSO_4

Calculate the formula mass for each compound. a. \(\mathrm{NO}_{2}\) b. \(\mathrm{C}_{4} \mathrm{H}_{10}\) c. \(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}\) d. \(\mathrm{Cr}\left(\mathrm{NO}_{3}\right)_{3}\) Text Transcription: NO_2 C_4H_10 C_6H_12O_6 Cr(NO_3)_3

Calculate the formula mass for each compound. a. \(\mathrm{MgBr}_{2}\) b. \(\mathrm{HNO}_{2}\) c. \(\mathrm{CBr}_{4}\) d. \(\mathrm{Ca}\left(\mathrm{NO}_{3}\right)_{2}\) Text Transcription: MgBr_2 HNO_2 CBr_4 Ca(NO_3)_2

Calculate the number of moles in each sample. a. 72.5 g \(\mathrm{CCl}_{4}\) b. 12.4 g \(\mathrm{C}_{12} \mathrm{H}_{22} \mathrm{O}_{11}\) c. 25.2 kg \(\mathrm{C}_{2} \mathrm{H}_{2}\) d. 12.3 g of dinitrogen monoxide Text Transcription: CCl_4 C_12H_22O_11 C_2H_2

Calculate the mass of each sample. a. 15.7 mol \(\mathrm{HNO}_{3}\) b. \(1.04 \times 10^{-3} \mathrm{~mol} \mathrm{} \mathrm{H}_{2} \mathrm{O}_{2}\) c. 72.1 mmol \(\mathrm{SO}_{2}\) d. 1.23 mol xenon difluoride Text Transcription: HNO_3 1.04x10^-3H_2O_2 SO_2

Determine the number of moles (of molecules or formula units) in each sample. a. 25.5 g \(\mathrm{NO}_{2}\) b. 1.25 kg \(\mathrm{CO}_{2}\) c. 38.2 g \(\mathrm{KNO}_{3}\) d. 155.2 kg \(\mathrm{Na}_{2} \mathrm{SO}_{4}\) Text Transcription: NO_2 CO_2 KNO_3 Na_2SO_4

Determine the number of moles (of molecules or formula units) in each sample. a. 55.98 g \(\mathrm{CF}_{2} \mathrm{Cl}_{2}\) b. 23.6 kg \(\mathrm{Fe}\left(\mathrm{NO}_{3}\right)_{2}\) c. 0.1187 g \(\mathrm{C}_{8} \mathrm{H}_{18}\) d. 195 kg CaO Text Transcription: CF_2Cl_2 Fe(NO_3)_2 C_8H_18

How many molecules are in each sample? a. 6.5 g \(\mathrm{H}_{2} \mathrm{O}\) b. 389 g \(\mathrm{CBr}_{4}\) c. 22.1 g \(\mathrm{O}_{2}\) d. 19.3 g \(\mathrm{C}_{8} \mathrm{H}_{10}\) Text Transcription: H_2O CBr_4 O_2 C_8H_10

How many molecules (or formula units) are in each sample? a. 85.26 g \(\mathrm{CCl}_{4}\) b. 55.93 kg \(\mathrm{NaHCO}_{3}\) c. 119.78 g \(\mathrm{C}_{4} \mathrm{H}_{10}\) d. \(4.59 \times 10^{3} \mathrm{~g} \mathrm{Na}_{3} \mathrm{PO}_{4}\) Text Transcription: CCl4 NaHCO3 C4H10 5.49x10^5Na3PO4

Calculate the mass (in g) of each sample. a. \(5.94 \times 10^{20} \mathrm{SO}_{3}\) molecules b. \(2.8 \times 10^{22} \mathrm{H}_{2} \mathrm{O}\) molecules c. 1 glucose molecule \(\left(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}\right)\) Text Transcription: 5.94 x 10^20 SO_3 2.8 x 10^22 H_2O C_6H_12O_6

Calculate the mass (in g) of each sample. a. \(4.5 \times 10^{25} \mathrm{O}_{3}\) molecules b. \(9.85 \times 10^{19} \mathrm{CCl}_{2} \mathrm{~F}_{2}\) molecules c. 1 water molecule Text Transcription: 4.5 x 10^25 O_3 9.85 x 10^19 CCl_2F_2

A sugar crystal contains approximately \(1.8 \times 10^{17}\) sucrose \(\left(\mathrm{C}_{12} \mathrm{H}_{22} \mathrm{O}_{11}\right)\) molecules. What is its mass in mg? Text Transcription: 1.8 x 10^17 (C_12H_22O_11)

A salt crystal has a mass of 0.12 mg. How many NaCl formula units does it contain?

Calculate the mass percent composition of carbon in each carbon-containing compound. a. \(\mathrm{CH}_{4}\) b. \(\mathrm{C}_{2} \mathrm{H}_{6}\) c. \(\mathrm{C}_{2} \mathrm{H}_{2}\) d. \(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{Cl}\) Text Transcription: CH_4 C_2H_6 C_2H_2 C_2H_5Cl

Calculate the mass percent composition of nitrogen in each nitrogen-containing compound. a. \(\mathrm{N}_{2} \mathrm{O}\) b. NO c. \(\mathrm{NO}_{2}\) d. \(\mathrm{HNO}_{3}\) Text Transcription: N_2O NO_2 HNO_3

Most fertilizers consist of nitrogen-containing compounds such as \(\mathrm{NH}_{3}\), \(\mathrm{CO}\left(\mathrm{NH}_{2}\right)_{2}\), \(\mathrm{NH}_{4} \mathrm{NO}_{31}\) and \(\left(\mathrm{NH}_{4}\right)_{2} \mathrm{SO}_{4}\). Plants use the nitrogen content in these compounds for protein synthesis. Calculate the mass percent composition of nitrogen in each of the fertilizers named in this problem. Which fertilizer has the highest nitrogen content? Text Transcription: NH_3 CO(NH_2)_2 NH_4NO_3 (NH_4)_2SO_4

Iron in the earth is in the form of iron ore. Common ores include \(\mathrm{Fe}_{2} \mathrm{O}_{3}\) (hematite), \(\mathrm{Fe}_{3} \mathrm{O}_{4}\) (magnetite), and \(\mathrm{FeCO}_{3}\) (siderite). Calculate the mass percent composition of iron for each of these iron ores. Which ore has the highest iron content? Text Transcription: Fe_2O_3 Fe_3O_4 FeCO_3

Copper(II) fluoride contains 37.42% F by mass. Calculate the mass of fluorine (in g) contained in 55.5 g of copper(II) fluoride.

Silver chloride, often used in silver plating, contains 75.27% Ag by mass. Calculate the mass of silver chloride required to plate 155 mg of pure silver.

The iodide ion is a dietary mineral essential to good nutrition. In countries where potassium iodide is added to salt, iodine deficiency (goiter) has been almost completely eliminated. The recommended daily allowance (RDA) for iodine is 150 \(\mu g\)/day. How much potassium iodide (76.45% I) must you consume to meet the RDA? Text Transcription: mu g

The American Dental Association recommends that an adult female should consume 3.0 mg of fluoride (\(\mathrm{F}^{-}\)) per day to prevent tooth decay. If the fluoride is consumed in the form of sodium fluoride (45.24% F), what amount of sodium fluoride contains the recommended amount of fluoride? Text Transcription: F^-

Write a ratio showing the relationship between the molar amounts of each element for each compound.

Write a ratio showing the relationship between the molar amounts of each element for each compound.

Determine the number of moles of hydrogen atoms in each sample. a. 0.0885 mol \(\mathrm{C}_{4} \mathrm{H}_{10}\) b. 1.3 mol \(\mathrm{CH}_{4}\) c. 2.4 mol \(\mathrm{C}_{6} \mathrm{H}_{12}\) d. 1.87 mol \(\mathrm{C}_{8} \mathrm{H}_{18}\) Text Transcription: C_4H_10 CH_4 C_8H_18 C_6H_12

Determine the number of moles of oxygen atoms in each sample. a. 4.88 mol \(\mathrm{H}_{2} \mathrm{O}_{2}\) b. 2.15 mol \(\mathrm{N}_{2} \mathrm{O}\) c. 0.0237 mol \(\mathrm{H}_{2} \mathrm{CO}_{3}\) d. 24.1 mol \(\mathrm{CO}_{2}\) Text Transcription: H_2O_2 N_2O H_2CO_3 CO_2

Calculate mass (in grams) of sodium in 8.5 g of each sodium-containing food additive. a. NaCl (table salt) b. \(\mathrm{Na}_{3} \mathrm{PO}_{4}\) (sodium phosphate) c. \(\mathrm{NaC}_{7} \mathrm{H}_{5} \mathrm{O}_{2}\) (sodium benzoate) d. \(\mathrm{Na}_{2} \mathrm{C}_{6} \mathrm{H}_{6} \mathrm{O}_{7}\) (sodium hydrogen citrate) Text Transcription: Na_3PO_4 NaC_7H_5O_2 Na_2C_6H_6O_7

Calculate the mass (in kilograms) of chlorine in 25 kg of each chlorofluorocarbon (CFC). a. \(\mathrm{CF}_{2} \mathrm{Cl}_{2}\) b. \(\mathrm{CFCl}_{3}\) c. \(\mathrm{C}_{2} \mathrm{FF}_{3} \mathrm{Cl}_{3}\) d. \(\mathrm{C} \mathrm{F}_{3} \mathrm{Cl}\) Text Transcription: CF_2Cl_2 CFCl_3 C_2F_3Cl_3 CF_3Cl

A chemist decomposes samples of several compounds; the masses of their constituent elements are shown. Calculate the empirical formula for each compound. a. 1.651 g Ag, 0.1224 g O b. 0.672 g Co, 0.569 g As, 0.486 g O c. 1.443 g Se, 5.841 g Br

A chemist decomposes samples of several compounds; the masses of their constituent elements are shown. Calculate the empirical formula for each compound. a. 1.245 g Ni, 5.381 g I b. 2.677 g Ba, 3.115 g Br c. 2.128 g Be, 7.557 g S, 15.107 g O

Calculate the empirical formula for each stimulant based on its elemental mass percent composition. a. nicotine (found in tobacco leaves): C 74.03%, H 8.70%, N 17.27% b. caffeine (found in coffee beans): C 49.48%, H 5.19%, N 28.85%, O 16.48%

Calculate the empirical formula for each natural flavor based on its elemental mass percent composition. a. methyl butyrate (component of apple taste and smell): C 58.80%, H 9.87%, O 31.33% b. vanillin (responsible for the taste and smell of vanilla): C 63.15%, H 5.30%, O 31.55%

The elemental mass percent composition of ibuprofen is 75.69% C, 8.80% H, and 15.51% O. Determine the empirical formula of ibuprofen.

The elemental mass percent composition of ascorbic acid (vitamin C) is 40.92% C, 4.58% H, and 54.50% O. Determine the empirical formula of ascorbic acid

A 0.77-mg sample of nitrogen reacts with chlorine to form 6.61 mg of the chloride. Determine the empirical formula of nitrogen chloride.

A 45.2-mg sample of phosphorus reacts with selenium to form 131.6 mg of the selenide. Determine the empirical formula of phosphorus selenide.

The empirical formula and molar mass of several compounds are listed. Find the molecular formula of each compound. a. \(\mathrm{C}_{6} \mathrm{H}_{7} \mathrm{N}\), 186.24 g/mol b. \(\mathrm{C}_{2} \mathrm{HCl}\), 181.44 g/mol c. \(\mathrm{C}_{5} \mathrm{H}_{10} \mathrm{NS}_{2}\), 296.54 g/mol Text Transcription: C_6H_7N C_2HCl C_5H_10NS_2

The molar mass and empirical formula of several compounds are listed. Find the molecular formula of each compound. a. \(\mathrm{C}_{4} \mathrm{H}_{9}\), 114.22 g/mol b. CCl, 284.77 g/mol c.\(\mathrm{C}_{3} \mathrm{H}_{2} \mathrm{N}\), 312.29 g/mol Text Transcription: C4H9 C3H2N

Combustion analysis of a hydrocarbon produced 33.01 g \(\mathrm{CO}_{2}\) and 13.51 g \(\mathrm{H}_{2} \mathrm{O}\). Calculate the empirical formula of the hydrocarbon. Text Transcription: CO_2 H_2O

Combustion analysis of naphthalene, a hydrocarbon used in mothballs, produced 8.80 g \(\mathrm{CO}_{2}\) and 1.44 g \(\mathrm{H}_{2} \mathrm{O}\). Calculate the empirical formula for naphthalene. Text Transcription: CO_2 H_2O

The foul odor of rancid butter is due largely to butyric acid, a compound containing carbon, hydrogen, and oxygen. Combustion analysis of a 4.30-g sample of butyric acid produces 8.59 g \(\mathrm{CO}_{2}\) and 3.52 g \(\mathrm{H}_{2} \mathrm{O}\). Determine the empirical formula for butyric acid. Text Transcription: CO_2 H_2O

Tartaric acid is the white, powdery substance that coats tart candies such as Sour Patch \(\text { Kids }^{\mathrm{TM}}\). Combustion analysis of a 12.01-g sample of tartaric acid—which contains only carbon, hydrogen, and oxygen—produces 14.08 g \(\mathrm{CO}_{2}\) and 4.32 g \(\mathrm{H}_{2} \mathrm{O}\). Determine the empirical formula for tartaric acid. Text Transcription: Kids^TM CO_2 H_2O

Classify each compound as organic or inorganic. a. \(\mathrm{CaCO}_{3}\) b. \(\mathrm{C}_{4} \mathrm{H}_{8}\) c. \(\mathrm{C}_{4} \mathrm{H}_{6} \mathrm{O}_{6}\) d. LiF Text Transcription: CaCO_3 C_4H_8 C_4H_6O_6

Classify each compound as organic or inorganic. a. \(\mathrm{C}_{8} \mathrm{H}_{18}\) b. \(\mathrm{CH}_{3} \mathrm{NH}_{2}\) c. CaO d. \(\mathrm{FeCO}_{3}\) Text Transcription: C_8H_18 CH_3NH2 FeCO_3

Determine whether each compound is a hydrocarbon.

Determine whether each compound is a hydrocarbon.

How many molecules of ethanol \(\left(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}\right)\) (the alcohol in alcoholic beverages) are present in 145 mL of ethanol? The density of ethanol is 0.789 g/\(\mathrm{cm}^{3}\). Text Transcription: (C_2H_5OH) cm^3

A drop of water has a volume of approximately 0.05 mL. How many water molecules does it contain? The density of water is 1.0 g/\(\mathrm{cm}^{3}\) . Text Transcription: cm^3

Determine the chemical formula of each compound and use it to calculate the mass percent composition of each constituent element. a. potassium chromate b. lead(II) phosphate c. cobalt(II) bromide

Determine the chemical formula of each compound and use it to calculate the mass percent composition of each constituent element. a. phosphorus pentachloride b. nitrogen triiodide c. carbon dioxide

A \(\text { Freon }{ }^{\mathrm{M}}\) leak in the air conditioning system of an old car releases 25 g of \(\mathrm{CF}_{2} \mathrm{Cl}_{2}\) per month. What mass of chlorine does this car emit into the atmosphere each year? Text Transcription: CF_2Cl_2 Freon^TM

A \(\text { Freon }{ }^{\mathrm{M}}\) leak in the air conditioning system of a large building releases 12 kg of \(\mathrm{CHF}_{2} \mathrm{Cl}\) per month. If the leak is allowed to continue, how many kilograms of Cl are emitted into the atmosphere each year? Text Transcription: Freon^TM CHF2Cl

A metal (M) forms a compound with the formula \(\mathrm{MCl}_{3}\). If the compound contains 65.57% Cl by mass, what is the identity of the metal? Text Transcription: MCl_3

A metal (M) forms an oxide with the formula \(\mathrm{M}_{2} \mathrm{O}\). If the oxide contains 16.99% O by mass, what is the identity of the metal? Text Transcription: M_2O

Estradiol is a female sexual hormone that causes maturation and maintenance of the female reproductive system. Elemental analysis of estradiol gives the following mass percent composition: C 79.37%, H 8.88%, O 11.75%. The molar mass of estradiol is 272.37 g/mol. Find the molecular formula of estradiol.

Fructose is a common sugar found in fruit. Elemental analysis of fructose gives the following mass percent composition: C 40.00%, H 6.72%, O 53.28%. The molar mass of fructose is 180.16 g/mol. Find the molecular formula of fructose.

Combustion analysis of a 13.42-g sample of equilin (which contains only carbon, hydrogen, and oxygen) produces 39.61 g \(\mathrm{CO}_{2}\) and 9.01 g \(\mathrm{H}_{2} \mathrm{O}\). The molar mass of equilin is 268.34 g/mol. Find its molecular formula. Text Transcription: H_2O CO_2

Estrone, which contains only carbon, hydrogen, and oxygen, is a female sexual hormone that occurs in the urine of pregnant women. Combustion analysis of a 1.893-g sample of estrone produces 5.545 g of \(\mathrm{CO}_{2}\) and 1.388 g \(\mathrm{H}_{2} \mathrm{O}\). The molar mass of estrone is 270.36 g/mol. Find its molecular formula. Text Transcription: H_2O CO_2

Epsom salts is a hydrated ionic compound with the following formula: \(\mathrm{MgSO}{ }_{4} \cdot x \mathrm{H}_{2} \mathrm{O}\). A 4.93-g sample of Epsom salts was heated to drive off the water of hydration. The mass of the sample after complete dehydration was 2.41 g. Find the number of waters of hydration (x) in Epsom salts. Text Transcription: MgSO_4 dot x H_2O

A hydrate of copper(II) chloride has the following formula: \(\mathrm{CuCl}_{2} \cdot \mathrm{x H}_{2} \mathrm{O}\). The water in a 3.41-g sample of the hydrate is driven off by heating. The remaining sample has a mass of 2.69 g. Find the number of waters of hydration (x) in the hydrate. Text Transcription: CuCl_2 dot x H_2O

A compound of molar mass 177 g/mol contains only carbon, hydrogen, bromine, and oxygen. Analysis reveals that the compound contains 8 times as much carbon as hydrogen by mass. Find the molecular formula.

Researchers obtain the following data from experiments to find the molecular formula of benzocaine, a local anesthetic, which contains only carbon, hydrogen, nitrogen, and oxygen. Complete combustion of a 3.54-g sample of benzocaine with excess \(\mathrm{O}_{2}\) forms 8.49 g of \(\mathrm{CO}_{2}\) and 2.14 g \(\mathrm{H}_{2} \mathrm{O}\). Another sample of mass 2.35 g is found to contain 0.199 g of N. The molar mass of benzocaine is found to be 165 g/mol. Find the molecular formula of benzocaine. Text Transcription: O_2 CO_2 H_2O

Find the total number of atoms in a sample of cocaine hydrochloride, \(\mathrm{C}_{17} \mathrm{H}_{22} \mathrm{CINO}_{4}\), of mass 23.5 mg. Text Transcription: C_17H_22CINO_4

Vanadium forms four different oxides in which the percent by mass of vanadium is, respectively, (a) 76%, (b) 68%, (c) 61%, and (d) 56%. Determine the formula and the name of each one of these oxides.

The chloride of an unknown metal is believed to have the formula \(\mathrm{MCl}_{3}\). A 2.395-g sample of the compound contains \(3.606 \times 10^{-2}\) mol Cl. Find the atomic mass of M. Text Transcription: MCl_3 3.606 x 10^-2

Write the structural formulas of two different compounds that each has the molecular formula \(\mathrm{C}_{4} \mathrm{H}_{10}\). Text Transcription: C_4H_10

A chromium-containing compound has the formula \(\mathrm{Fe}_{x} \mathrm{Cr}_{y} \mathrm{O}_{4}\) and is 28.59% oxygen by mass. Find x and y. Text Transcription: Fe_xCr_yO_4

A phosphorus compound that contains 34.00% phosphorus by mass has the formula \(\mathrm{X}_{3} \mathrm{P}_{2}\). Identify the element X. Text Transcription: X_3P_2

A particular brand of beef jerky contains 0.0552% sodium nitrite by mass and is sold in an 8.00-oz bag. What mass of sodium does the sodium nitrite contribute to the sodium content of the bag of beef jerky?

Phosphorus is obtained primarily from ores containing calcium phosphate. If a particular ore contains 57.8% calcium phosphate, what minimum mass of the ore must be processed to obtain 1.00 kg of phosphorus?

A mixture of NaCl and NaBr has a mass of 2.00 g and contains 0.75 g of Na. What is the mass of NaBr in the mixture?

Three pure compounds form when 1.00-g samples of element X combine with, respectively, 0.472 g, 0.630 g, and 0.789 g of element Z. The first compound has the formula \(X_{2} Z_{3}\). Find the empirical formulas of the other two compounds. Text Transcription: X_2Z_3

A mixture of \(\mathrm{CaCO}_{3}\) and \(\left(\mathrm{NH}_{4}\right)_{2} \mathrm{CO}_{3}\) is 61.9% \(\mathrm{CO}_{3}\) by mass. Find the mass percent of \(\mathrm{CaCO}_{3}\) in the mixture. Text Transcription: CaCO_3 (NH_4)_2CO_3 CO_3

A mixture of 50.0 g of S and \(1.00 \times 10^{2}\) g of \(\mathrm{Cl}_{2}\) reacts completely to form \(\mathrm{S}_{2} \mathrm{Cl}_{2}\) and \(\mathrm{SCl}_{2}\). What mass of \(\mathrm{S}_{2} \mathrm{Cl}_{2}\) forms? Text Transcription: 1.00 x 10^2 Cl_2 S_2Cl_2 SCl_2

Because of increasing evidence of damage to the ozone layer, chlorofluorocarbon (CFC) production was banned in 1996. However, there are about 100 million auto air conditioners in operation that still use CFC-12 \(\left(\mathrm{CF}_{2} \mathrm{Cl}_{2}\right)\). These air conditioners are recharged from stockpiled supplies of CFC-12. If each of the 100 million automobiles contains 1.1 kg of CFC-12 and leaks 25% of its CFC-12 into the atmosphere per year, how much chlorine, in kg, is added to the atmosphere each year due to auto air conditioners? (Assume two significant figures in your calculations.) Text Transcription: CF_2Cl_2

A particular coal contains 2.55% sulfur by mass. When the coal is burned, it produces \(\mathrm{SO}_{2}\) emissions, which combine with rainwater to produce sulfuric acid. Use the formula of sulfuric acid to calculate the mass percent of S in sulfuric acid. Then determine how much sulfuric acid (in metric tons) is produced by the combustion of 1.0 metric ton of this coal. (A metric ton is 1000 kg.) Text Transcription: SO_2

Lead is found in Earth’s crust as several different lead ores. Suppose a certain rock is 38.0% PbS (galena), 25.0% \(\mathrm{PbCO}_{3}\) (cerussite), and 17.4% \(\mathrm{PbSO}_{4}\) (anglesite). The remainder of the rock is composed of substances containing no lead. How much of this rock (in kg) must be processed to obtain 5.0 metric tons of lead? (A metric ton is 1000 kg.) Text Transcription: PbSO_4 PbCO_3

A 2.52-g sample of a compound containing only carbon, hydrogen, nitrogen, oxygen, and sulfur is burned in excess oxygen to yield 4.23 g of \(\mathrm{CO}_{2}\) and 1.01 g of \(\mathrm{H}_{2} \mathrm{O}\). Another sample of the same compound, of mass 4.14 g, yields 2.11 g of \(\mathrm{SO}_{3}\). A third sample, of mass 5.66 g, yields 2.27 g of \(\mathrm{HNO}_{3}\). Calculate the empirical formula of the compound. (Hint: Use the first set of data to determine % C and % H by mass. Use the second and third sets of data to determine % S and % N by mass. Then determine % O by mass by difference from 100%.) Text Transcription: CO_2 H_2O SO_3 HNO_3

A compound of molar mass 229 contains only carbon, hydrogen, iodine, and sulfur. Analysis shows that a sample of the compound contains 6 times as much carbon as hydrogen, by mass. Calculate the molecular formula of the compound.

The elements X and Y form a compound that is 40% X and 60% Y by mass. The atomic mass of X is twice that of Y. What is the empirical formula of the compound?

A compound of X and Y is \(\frac{1}{3} X\) by mass. The atomic mass of element X is one-third the atomic mass of element Y. Find the empirical formula of the compound. Text Transcription: 1/3 X

A mixture of carbon and sulfur has a mass of 9.0 g. Complete combustion with excess \(\mathrm{O}_{2}\) gives 23.3 g of a mixture of \(\mathrm{CO}_{2}\) and \(\mathrm{SO}_{2}\). Find the mass of sulfur in the original mixture. Text Transcription: O_2 CO_2 SO_2

When molecules are represented by molecular models, what does each sphere represent? How big is the nucleus of an atom in comparison to the sphere used to represent an atom in a molecular model?

Without doing any calculations, determine which element in each of the compounds will have the highest mass percent composition. a. CO b. \(\mathrm{N}_{2} \mathrm{O}\) c. \(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}\) d. \(\mathrm{NH}_{3}\) Text Transcription: N_2O C_6H_12O_6 NH_3

Explain the problem with this statement and correct it: “The chemical formula for ammonia \(\left(\mathrm{NH}_{3}\right)\) indicates that ammonia contains 3 grams of hydrogen to each gram of nitrogen.” Text Transcription: (NH_3)

Without doing any calculations, arrange the elements in \(\mathrm{H}_{2} \mathrm{SO}_{4}\) in order of decreasing mass percent composition. Text Transcription: H_2SO_4

Discuss these questions with the group and record your consensus answer. Using group members to play the roles of nuclei and electrons, demonstrate the formation of an ionic bond between Na and Cl. Demonstrate the formation of the covalent bonds in \(\mathrm{H} 2 \mathrm{O}\). Text Transcription: H_2O

Discuss these questions with the group and record your consensus answer. Create a flowchart with a series of simple questions that can be used to determine whether a chemical formula is that of an atomic element, a molecular element, a molecular compound, or an ionic compound. Use your flowchart to identify the correct category for \(\mathrm{P}_{4}\), KCl, \(\mathrm{CH}_{4}\), Ne, and \(\mathrm{NH}_{4} \mathrm{NO}_{3}\). Text Transcription: P_4 CH_4 NH_4NO_3

Discuss these questions with the group and record your consensus answer. Have each member of your group list one similarity or difference between the naming conventions for ionic and the naming conventions of molecular compounds.

Discuss these questions with the group and record your consensus answer. A compound isolated from the rind of lemons is 88.14% carbon and 11.86% hydrogen by mass. How many grams of C and H are there in a 100.0-g sample of this substance? How many moles of C and H? What is the empirical formula? The molar mass is determined to be 136.26 g/mol. What is the molecular formula? Which step of the process just described does your group understand the least? Which step will be most challenging for the members of your group to remember?

The amount of carbon dioxide in the atmosphere has been increasing over the past century as a result of the combustion of fossil fuels (coal, oil, and natural gas). Carbon dioxide is a greenhouse gas that plays a significant role in climate. The increase in carbon dioxide is correlated with changes in climate that have climate scientists concerned. The graph shown here illustrates the increase in atmospheric carbon dioxide from 1860 to the present. Study the graph and answer the questions that follow. a. By how much did the level of carbon dioxide (in ppmv) increase between 1880 and the present day? b. What is the percent increase in the level of carbon dioxide between 1880 and the present day? c. Assuming that the total volume of air in the atmosphere around Earth is \(5.1 \times 10^{9} \mathrm{km}^{3}\) and that the concentration of \(\mathrm{CO}_{2}\) is uniform throught this volume, what is the present-day volume of \(\mathrm{CO}_{2}\) in the atmosphere? d. Determine the percentage average yearly increase in atmospheric \(\mathrm{CO}_{2}\) from 1960 to the present day. e. If atmospheric carbon dioxide continues to increase at the rate you determined in part d, what will its concentration (in ppmv) be in the year 2040? Text Transcription: 5.1 x 10^9 km^3 CO_2